This document discusses acids, bases, and pH. It defines Arrhenius and Bronsted-Lowry acids and bases. Strong acids like HCl fully dissociate in water, while weak acids like H3PO4 only partially dissociate. The pH scale measures hydrogen ion concentration from 0-14. Buffers resist changes in pH using a weak acid and its conjugate base. Hydrolysis of salts can affect pH depending on if they are made from strong or weak acids and bases.
Acids are divided into two categories based on the ease with which they can donate protons to the solvent: i) strong acids and ii) weak acids
Strong acids are acids that completely dissociate in water. The reaction of an acid with its solvent (typically H2O) is called an acid dissociation reaction.
Weak acids are acids that dissociate partially in water. The extent of dissociation is given by the equilibrium constant.
Note:
A measure of the relative strength of an acid is: i) the equilibrium constant ka of the dissociation reaction of the acid in water (depends on temperature) ii) the degree of dissociation α of the acid in water (depends on the concentration of the acid an on temperature).
Acids bases and buffers
Pharmaceutical Inorganic Chemistry
Unit 2, Chapter 1
Arrhenius, Bronsted-Lowry and Lewis Concepts of Acids and bases,
Concept of pH, pOH, pKa, pKb
Concept of buffers, buffer solutions, buffer action, and buffer capacity,
Buffer equation
Buffers in pharmaceuticals
Buffered isotonic solutions
Measurement and adjustment of tonicity
Acids are divided into two categories based on the ease with which they can donate protons to the solvent: i) strong acids and ii) weak acids
Strong acids are acids that completely dissociate in water. The reaction of an acid with its solvent (typically H2O) is called an acid dissociation reaction.
Weak acids are acids that dissociate partially in water. The extent of dissociation is given by the equilibrium constant.
Note:
A measure of the relative strength of an acid is: i) the equilibrium constant ka of the dissociation reaction of the acid in water (depends on temperature) ii) the degree of dissociation α of the acid in water (depends on the concentration of the acid an on temperature).
Acids bases and buffers
Pharmaceutical Inorganic Chemistry
Unit 2, Chapter 1
Arrhenius, Bronsted-Lowry and Lewis Concepts of Acids and bases,
Concept of pH, pOH, pKa, pKb
Concept of buffers, buffer solutions, buffer action, and buffer capacity,
Buffer equation
Buffers in pharmaceuticals
Buffered isotonic solutions
Measurement and adjustment of tonicity
Slides giving an overview on pH and its measurement.
Contains information about pH meters, its calibration, maintenance , types of ph electrode and modern definition of pH
Slides giving an overview on pH and its measurement.
Contains information about pH meters, its calibration, maintenance , types of ph electrode and modern definition of pH
Chapter No 1 : Acids, Bases and BuffersChetan Jain
This is chapter No 1 of Pharmaceutical Chemistry - I for Diploma in Pharmacy (D. Pharmacy)
Details notes for Diploma in Pharmacy (D.Pharmacy) Students.
Acids, Bases And Buffers Pharmaceutical Inorganic chemistry UNIT-II (Part-I)
Acids, Bases are defined by Four main theories,
1.Traditional theory / concept
2.Arrhenius theory
3.Bronsted and Lowry theory
4.Lewis theory
Importance of acids and bases in pharmacy
Buffers: Buffer action
Buffer capacity Buffers system
Types of Buffers : Generally buffers are of two types:
1. Acidic buffers
2. Basic buffers
There are some other buffer system:
3. Two salts acts as acid-base pair. Ex- Potassium hydrogen phosphate and potassium dihydrogen phosphate.
4. Amphoteric electrolyte. Ex- Solution of glycine.
5. Solution of strong acid and solution of strong base. Ex- Strong HCl with KCl Mechanism of Buffer action: Mechanism of Action of acidic buffers: Buffer equation-Henderson-Hasselbalch equation:
Standard Buffer Solutions Preparation of Buffer Solutions: Buffers in pharmaceutical systems or Application of buffer: Stability of buffers Buffered isotonic solution Types of Buffer Isotonic solution
1. Isotonic Solutions:
2. Hypertonic Solutions:
3. Hypotonic Solution:
Measurement of Tonicity: 1. Hemolytic method: 2. Cryoscopic method or depression of freezing point:
Methods of adjusting the tonicity:
Class I methods:
In this type, sodium chloride or other substances are added to the solution in sufficient quantity to make it isotonic. Then the preparation is brought to its final volume withan isotonic or a buffered isotonic diluting solution.
These methods are of two types:
Cryoscopic method
Sodium chloride equivalent method.
Class II methods:
In this type, water is added in sufficient quantity make the preparation isotonic. Then the preparation is brought to its volume with an isotonic or a buffered isotonic diluting solution.
These methods are of two types:
White-Vincent method
Sprowls method.
Introduction/ Concept of acid and base, Importance of acids and bases in Pharmacy, storage condition. Official acids: Phosphoric acid (Conc/dil), HCl (Conc/dil), Boric acid. Official Bases: NaOH, KOH, Ca (OH)2, dil. and strong NH3, Na2CO3, Acidosis and Alkalosis.
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Cheryl Hung, ochery.com
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Topics covered:
UI automation Introduction,
UI automation Sample
Desktop automation flow
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Deepak Rai, Automation Practice Lead, Boundaryless Group and UiPath MVP
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Learn about:
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• Test Automation: How AI-powered test case generation, optimization, and self-healing tests are making testing more efficient and effective.
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Sectoral targets and attacks as well as the cost of ransom
Global APT activity, AI usage, actor and tactic profiles, and implications
Rise in volumes of AI-powered cyberattacks
Major cyber events in 2024
Malware and malicious payload trends
Cyberattack types and targets
Vulnerability exploit attempts on CVEs
Attacks on counties – USA
Expansion of bot farms – how, where, and why
In-depth analysis of the cyber threat landscape across North America, South America, Europe, APAC, and the Middle East
Why are attacks on smart factories rising?
Cyber risk predictions
Axis of attacks – Europe
Systemic attacks in the Middle East
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2. Heatmap utilization for testing
3. Optimization of testing processes
4. Demo
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Execution from the test manager
Orchestrator execution result
Defect reporting
SAP heatmap example with demo
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https://arxiv.org/abs/2306.08302
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Do you want to learn how to model and simulate an electrical network from scratch in under an hour?
Then welcome to this PowSyBl workshop, hosted by Rte, the French Transmission System Operator (TSO)!
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- Visualization tools to display your network;
- Grid simulation tools, such as power flows, security analyses (with or without remedial actions) and sensitivity analyses;
The framework is mostly written in Java, with a Python binding so that Python developers can access PowSyBl functionalities as well.
What you will learn during the webinar:
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LF Energy Webinar: Electrical Grid Modelling and Simulation Through PowSyBl -...
Acids, Bases, Buffers, Electrolytes, & pH
1. Acids, Bases, Buffers,
Electrolytes, and pH
•
This chapter has very big
applications with biological
systems and the environment.
•
We have had a good
introduction to this with the
acid-base titration that we did
during the solutions chapter.
Damage from Acid Rain
2. A Quick Quiz...
• Name the following:
• HCl, HI, H SO , HNO , H PO
2 4 3 3 4
• Write formulas for the following
• Hydrobromic acid, Acetic acid,
Carbonic acid, Sulfuric acid,
Hypochlorous acid
3. How Did You Do?
• Hydrochloric acid, Hydroiodic acid,
Sulfuric acid, Nitric acid, Phosphoric acid
• HBr, HC H O , H CO , H SO , HClO
2 3 2 2 3 2 4
4. Definitions of Acids and Bases
1. Arrhenius acid- dissociates to produce H3O+ (H+)
when dissolved in water.
2. Arrhenius base- produces OH- when dissolved in
water
3. Bronsted-Lowry Acid- anything that donates a
proton
4. Bronsted-Lowry Base- anything that accepts a
proton
HCl
+
NH3
NH4Cl
Proton
Proton Svante Arrhenius
Donor
Acceptor
5. Dissociation- the extent to which
protons are produced or accepted
Acid
Strength
HCl
1
H2SO4
2
H3PO4
3
While H3PO4 has two more hydrogens than HCl, it does not
dissociate to the same extent.
Strong
Weak
Acids: HCl, H2SO4, HNO3
Acids: H3PO4, HC2H3O2, H2CO3
Bases: NaOH, KOH, Ba(OH)2
Bases: NH4OH, Mg(OH)2
6. Another Quick Quiz...
• Which pH value is acidic?
• pH 7.0; 5.0; or 8.0
• Why is HCl a stronger acid than H PO ?
3 4
7. How did you do?
• pH 5.0!
• HCl dissociates more than H PO
3 4
8. The pH scale: Pouvoir
Hydrogen (Power of
Hydrogen)
Acid 1----------------------------------7------------------------------------14 Base
-log of the hydrogen ion concentration (Molarity)
Calculations:
pH 2.56 = 10-2.56
(2nd function;10x;change sign;2.5)
= 2.75 x 10-3 M [H+]
9. Buffers: made from a weak acid and a
salt containing the acid’s conjugate
base.
Carbonate-Bicarbonate Buffer in Humans
An application of
Le Chatelier’s
Principle
HC2H3O2 + NaC2H3O2 <->
H+ + C2H3O2- + Na+ + C2H3O2-
Stress
Result
Add NaOH
Shift right: forms water, dissociates HC2H3O2
Add HCl
Shift left: forms HC2H3O2, undissociated
10. Hydrolysis
Hydrolysis of salts and pH:
Salt
Made From
pH
NH4NO3
weak base/strong acid
4-5
KCl
strong base/strong acid
7
NaC2H3O2
strong base/weak acid
9-10
MgCO3
weak base/weak acid
7
